A student wrote the following equation C6H12O6(s) + 602(g) → 6CO₂(g) + 6H₂O(g) + energy Based on the fact that water vapour is a product, the logical conclusion is that the equation represents: Select one: Ophotosynthesis in an open system cellular respiration in a closed system combustion in a closed system combustion in an open system

A student wrote the following equation C6H12O6(s) + 602(g) → 6CO₂(g) + 6H₂O(g) + energy Based on the fact that water vapour is a product, the logical conclusion is that the equation represents: Select one: Ophotosynthesis in an open system cellular respiration in a closed system combustion in a closed system combustion in an open system

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 1.37 g sample of butane, C4H10(g), was burned in a bomb calorimeter in the presence of excess oxygen. The calorimeter contained 1.09 kg of water. Calculate the heat exchanged with respect to the system during the reaction if the calorimeter has a heat capacity of 648. J/°C and the temperature of the calorimeter and water changed from 23.6°C to 35.6°C? Enter your answer to 3 significant figures in decimal form. Do not enter units since they are already given. 58.12 kJ Calculate the heat exchanged with respect to the system per mole of butane. Enter your answer to 3 signficant figures in decimal form. Do not enter units since they are already given.’ 2547.5 kJ
A student dissolves 12.8 g of ammonium nitrate (NH4NO₂) in 200. g of water in a well-insulated open cup. She then observes the temperature of the water fall from 22,0 °C to 16.5 °C over the course of 5.6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH NO3(s)→ NH(aq) + NO3(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 2 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NH NO rxn exothermic…
Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction. If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?
When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.64g of glucose is burned in a calorimeter containing 788 g of water, and the temperature of the assembly increases from 20.10oC to 24.16oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol.
Measurements show that the energy of a mixture of gaseous reactants decreases by 373. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 136. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Round your answer to 3 x10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic
A 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.47oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)
Constants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HCI(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 51.5 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22,1°C to 24.1 C Part A Find A H,xn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4. 18 J/g. C as the specific heat capacity.) 國 AHxn = kJ/mol Submit Request Answer Provide Feedback Next> P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Pollcy Permissions | Contact Us Vi 1:23
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)
Calculate ΔHo for the process ½ N2(g) + ½ O2(g) → NO(g) from the following information N2(g) + 2 O2(g) → 2 NO2(g) ΔHo = -105.8 kJ/mol 2 NO(g) + O2 → 2 NO2(g) ΔHo = -216.7 kJ/mol
Consider the reaction: 8 H2O (l) + 4CO2 (g)→4 CH3OH (l) + 6 O2 (g) ΔH = +2905.6 kJ What is ΔH for the following reaction? 2 CH3OH (l) + 3 O2 (g) →4 H2O (l) + 2 CO2 (g)